Double Replacement Reactions: Complete and balance. Identify the precipitate (highlight it!!)?

1 Answer
anor277
May 24, 2017

In aqueous solution we would expect ionization of the individual reagents.......

Explanation:

(i) Ag^(+) + Cl^(-)rarrAgCl(s)darr

AgCl is as soluble as a brick. The state is indicated by (s), i.e. "solid"; some chemists put a down arrow as shown to emphasize its precipitation.

ELSE,

2AgNO_3(aq) + MgCl_2(aq) rarr 2AgCl(s) darr +Mg(NO_3)_2(aq)

The magnesium ions, and the nitrate ions are thus along for the ride and do not participate in MACROSCOPIC chemical change.

(ii) Fe^(2+) + HO^(-)rarrFe(OH)_2(s)darr

ELSE,

FeCl_2(aq) + 2NaOH(aq) rarr Fe(OH)_2(s) darr +2NaCl(aq)

The sodium ions, and the chloride ions are thus along for the ride and do not participate in MACROSCOPIC chemical change.

(iii) CO_3(aq)^(2-) + Fe^(2+)rarrFeCO_3(s)darr

ELSE,

Na_2CO_3(s) + FeSO_4(aq) rarr 2FeCO_3(s) darr +Na_2(SO_4)(aq)

Upon dissolution of the salts in an aqueous medium; SOME of the ions are spectator ions and thus do not participate in reaction. The given net ionic equations reflect the macroscopic chemical change.

Related questions
See all questions in Double Replacement Reactions
Impact of this question
2472 views around the world
You can reuse this answer
Creative Commons License